# Problem: Given the following information:A+B ---&gt; 2D Delta H= -707.5 kJ, Delta S= 338.0 J/KC ---&gt; D Delta H= 504.0 kJ, Delta S= -244.0 J/KCalculate Delta G for the following reaction at 298K.A+B ---&gt;2C

###### FREE Expert Solution

We can use the following equation to solve for ΔG˚rxn of the first 2 reacitons:

$\overline{){\mathbf{\Delta G}}{{\mathbf{°}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{\Delta H}}{{\mathbf{°}}}_{{\mathbf{rxn}}}{\mathbf{-}}{\mathbf{T\Delta S}}{{\mathbf{°}}}_{{\mathbf{rxn}}}}$

We’re given the ΔH˚rxn and ΔS˚rxn of the reaction 1 (A+B → 2D) :

ΔH˚rxn =  -707.5 kJ

ΔS˚rxn = 338.0 J/K

94% (44 ratings) ###### Problem Details

Given the following information:

A+B ---> 2D Delta H= -707.5 kJ, Delta S= 338.0 J/K

C ---> D Delta H= 504.0 kJ, Delta S= -244.0 J/K

Calculate Delta G for the following reaction at 298K.

A+B --->2C

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